Consider the following reaction: co2(g)+ccl4(g)⇌2cocl2(g) calculate δg for this reaction at25 ∘c under these conditions: pco2pccl4pcocl2===0.100atm0.180atm0 .735atm δg∘f for co2(g) is −394.4kj/mol, δg∘f for ccl4(g) is −62.3kj/mol, and δg∘f for cocl2(g) is −204.9kj/mol.

The for the reaction is 55.328 kJ/mol

Explanation:

For the given balanced chemical equation:

We are given:

To calculate for the reaction, we use the equation:

For the given equation:

Putting values in above equation, we get:

Conversion factor used = 1 kJ = 1000 J

The expression of for the given reaction:

We are given:

Putting values in above equation, we get:

To calculate the Gibbs free energy of the reaction, we use the equation:

where,

= Gibbs' free energy of the reaction = ?

= Standard gibbs' free energy change of the reaction = 46900 J

R = Gas constant =

T = Temperature =

= equilibrium constant in terms of partial pressure = 30.0125

Putting values in above equation, we get:

Hence, the for the reaction is 55.328 kJ/mol

answers: to make sure that all of the broken pieces of tablet were added to the water, to allow for fair comparison of all three trials, with different particle sizes to avoid experimental error

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